Chapter 10

Of the following elements, which possesses the highest electron affinity ? (a) As (b) \(\mathrm{O}\) (c) \(\mathrm{S}\) (d) Se

A large difference between the fourth and fifth ionization energies indicates the presence of (a) 5 valence electrons in an atom (b) 6 valence electrons in an atom (c) 4 valence electrons in an atom (d) 8 valence electrons in an atoin

Electron affinity is defined as the (a) Energy required to remove an electron from an isolated gaseous atom (b) Energy released when an electron is added to an isolated atom in the gaseous state (c) Energy required to add an electron to an isolated atom in the gaseous state (d) Ability of an atom to attract an electron

Which of the following elements never has an oxidation state of \(+1 ?\) (a) \(\underline{F}\) (b) \(\mathrm{C}]\) (c) \(\mathrm{Br}\) (d) I

Representative elements belong to (a) s- and \(p\)-block (b) d-block (c) d- and \(f\)-block (d) f-block

An element is called Ununbium. What is its atomic number? (a) 102 (b) 112 (c) 98 (d) 108

The atomic sizes are not significantly different for which series of elements? (a) \(\mathrm{Bi}, \mathrm{Na}, \mathrm{K}, \mathrm{Rb}\) (b) \(\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}, \mathrm{Si}\) (c) \(\mathrm{O}, \mathrm{S}, \mathrm{Sc}, \mathrm{Te}\) (d) \(\mathrm{Cr}, \mathrm{Mn}, \mathrm{Fe}, \mathrm{Co}\)

Which block elements show variable valency? (a) 's' and 'p' block (b) "s' and 'd' block (c) 'p' and ' \(\mathrm{d}^{\prime}\) block (d) none of these

Inert pair effect is shown by (a) s-block (b) p-block (c) d-block (d) \(f\)-block

If the aufbau principle had not been followed, \(\mathrm{Ca}(Z=20)\) would have been placed in the (a) s-block (b) \(p\)-block (c) d-block (d) \(f\)-block

Electron affinity is positive when (a) \(\mathrm{O}^{-}\)is formed from \(\mathrm{O}\) (b) \(\mathrm{O}^{2-\text { is formed }}\) form \(\mathrm{O}^{-}\) (c) \(\mathrm{O}^{*}\) is formed from \(\mathrm{O}\) (d) Electron affinity is always a negative value

Which of the following will have maximum electron affinity ? (a) \(1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{5}\) (b) \(\mathrm{ls}^{2} 2 \mathrm{~s}^{2} 2 p^{6}\) (c) \(1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 p^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{5}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\)

Which pair is different from the others (a) \(\mathrm{Li}-\mathrm{Mg}\) (b) \(\mathrm{Na}-\mathrm{K}\) (c) \(\mathrm{Ca}-\mathrm{Mg}\) (d) \(\mathrm{B}-\mathrm{Al}\)

The atom with lowest atomic number that has a ground state electronic configuratio of \((n-1) d^{5} n s^{2}\) is in the (a) 2nd period (b) 3rd period (c) 4 th period (d) 5 th period

Which pair is different from the others (a) Li-Mg (b) \(\mathrm{B}-\mathrm{Si}\) (c) \(\mathrm{Be} \cdot \mathrm{AI}\) (d) \(\mathrm{L}_{1} \mathrm{Na}\)

Which one of the following arrangements not truly represent the property inlin ated ayainst it? (a) \(\mathrm{Br}_{2}<\mathrm{Cl}_{2}<\mathrm{F}_{2}\) : Electro negativity (b) \(\mathrm{Br}_{2}<\mathrm{F}_{2}<\mathrm{Cl}_{4}\) : I lectron affinity (c) \(\mathrm{Br}_{2}<\mathrm{Cl}_{2}<\mathrm{F}_{2}:\) Bond energy (d) \(\mathrm{Br}_{2}<\mathrm{Cl}_{2}<\mathrm{I}_{1}\), Onidirimg priwer

The formation of the oxide ion \(O^{\prime}(g)\) require first an exothermic and then an endothermic \(O(g)+e^{-} O^{2-}(g) ; H P=844 \mathrm{~kJ} \mathrm{~mol}^{-1}\) This is because (a) Oxygen is more electronegative (b) \(O^{-}\)ion has comparatively larger size than oxygen atom (c) \(O^{-}\)ion will tend to resist the addition of another electron (d) Oxygen has high electron affinity

Among \(\mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{SiO}_{2}, \mathrm{P}_{2} \mathrm{O}_{3}\) and \(\mathrm{SO}_{2}\) the correct order of acid strength is (a) \(\mathrm{SO}_{2}<\mathrm{P}_{2} \mathrm{O}_{3}<\mathrm{SiO}_{2}<\mathrm{Al}_{2} \mathrm{O}_{3}\) b) \(\mathrm{Al}_{2} \mathrm{O}_{3}<\mathrm{SiO}_{2}<\mathrm{P}_{2} \mathrm{O}_{3}<\mathrm{SO}_{2}\) (c) \(\mathrm{Al}_{2} \mathrm{O}_{3}<\mathrm{SiO}_{2}<\mathrm{SO}_{2}<\mathrm{P}_{2} \mathrm{O}_{3}\) d) \(\mathrm{SiO}_{2}<\mathrm{SO}_{2}<\mathrm{Al}_{2} \mathrm{O}_{3}<\mathrm{P}_{2} \mathrm{O}_{3}\)

The incorrect statement among the following is (a) The first ionization potential of \(\mathrm{Al}\) is less than the first ionization potential of \(\mathrm{M}_{\mathrm{g}}\) (b) The second ionization potential of \(\mathrm{Mg}\) is greater than the second ionization potential of \(\mathrm{Na}\). (c) The first ionization potential of \(\mathrm{Na}\) is less than the first ionization potential of \(\mathrm{Mg}\) (d) The third ionization potential of \(\mathrm{Mg}\) is greater than the third ionization potential of Al

Amongst the following elements (whose electronic configurations are givell belown: one having the highest ionization energy is (a) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p}^{1}\) (b) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p}^{3}\) (c) \(\left[\mathrm{Ne} \mid 3 \mathrm{~s}^{2} 3 \mathrm{p}^{2}\right.\) (d) \([\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2} 4 \mathrm{p}^{2}\)

Four successive members of the first row transition elements are listed below with then atomic numbers. Which one of them is expected to have the highest third ionization enerig \(?\) (a) Vanadium \((Z=23)\) (b) Chromium \((Z=24)\) (c) Iron \((Z=26)\) (d) Manganese \((Z=35)\)

A sudden jump between the values of second and third ionization energies of element would be associated with which of the following electronic configurations. (a) \(1 s^{2} 2 s^{2} 2 v^{6} 3 s^{1}\) (b) \(1 s^{2}=^{2} 2 p^{6} 3 s^{2} 3 p^{\prime}\) (c) \(1 \mathrm{~s}^{2} 2 s^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{1} 3 \mathrm{p}^{2}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}\)

For electron affinity of halogen which of the following is correct ? mer \(>\mathrm{F}\) (b) \(\mathrm{F}>\mathrm{Cl}\) (c) \(\mathrm{Br}>\mathrm{Cl}\) (d) \(\mathrm{F}>1\)

In which of the following arrangements, the order is not according to the propert: indicated against it ? (a) \(\mathrm{Al}^{3+}<\mathrm{Mg}^{2 *}<\mathrm{Na}^{+}<\mathrm{F}\) Increasing ionic size (b) \(\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}\) Increasing first ionization energy (c) \(\mathrm{I}<\mathrm{Br}<\mathrm{F}<\mathrm{Cl}\) Increasing electron gain enthalpy (without negative sign) (d) \(L_{i}<\mathrm{Na}<\mathrm{K}<\mathrm{Rb}\) Increasing metallic radius

Which of the following is known as the bridge element of 2 nd group in \(\underline{\text { Mendeleev's table ? }}\) (a) \(\mathrm{Zn}\) (b) \(\underline{\mathrm{Sr}}\) (c) \(\mathrm{Mg}\) (d) \(\mathrm{Hg}\)

The successive ionization energies in kJ/mol of an element \(\mathrm{P}\) are \(740,1500,7000,10500\), \(13600,18000,21700 .\) Which ion is the most likely to be formed when \(X\) reacts with chloride ? (a) \(\underline{p^{2}}\) (b) \(\mathrm{P}^{+}\) (c) \(\mathrm{P}^{+2}\) (d) \(\mathrm{P}^{+3}\)